Electrochemical Polishing of Silverware: A Demonstration of Voltaic and Galvanic CellsMichelle M. Ivey and Eugene T. SmithUsing a battery and a graphite electrode, an electrolytic cell is constructed to generate a layer of tarnish on silverware. Students then determine that the tarnish can be removed by electrochemically converting it back to silver using aluminum foil and baking soda.Ivey, Michelle M.; Smith, Eugene T. J. Chem. Educ.2008, 85, 68.

Lithium Batteries: A Practical Application of Chemical PrinciplesRichard S. TreptowIn recent years batteries have emerged in the marketplace that take advantage of the unique properties of lithium. Lithium metal is an attractive choice to serve as a battery anode because it is easily oxidized and it produces an exceptionally high amount of electrical charge per unit-weight.Treptow, Richard S. J. Chem. Educ.2003, 80, 1015.

Consumer Chemistry |

Electrochemistry |

Oxidation / Reduction |

Electrolytic / Galvanic Cells / Potentials |

Applications of Chemistry

Lithium Batteries: A Practical Application of Chemical PrinciplesRichard S. TreptowIn recent years batteries have emerged in the marketplace that take advantage of the unique properties of lithium. Lithium metal is an attractive choice to serve as a battery anode because it is easily oxidized and it produces an exceptionally high amount of electrical charge per unit-weight.Treptow, Richard S. J. Chem. Educ.2003, 80, 1015.

Consumer Chemistry |

Electrochemistry |

Oxidation / Reduction |

Electrolytic / Galvanic Cells / Potentials |

Applications of Chemistry

Why Do Some Batteries Last Longer Than Others?Michael J. Smith and Colin A. VincentComparing the energy content of the cathode material of different commercial batteries using a test cell.Smith, Michael J.; Vincent, Colin A. J. Chem. Educ.2002, 79, 851.

Structure and Content of Some Primary BatteriesMichael J. Smith and Colin A. VincentAn experiment that complements electrochemical characterization and allows students to explore the structure of commercial cells and calculate the anode and cathode capacities from the stoichiometry of the cell reaction.Smith, Michael J.; Vincent, Colin A. J. Chem. Educ.2001, 78, 519.

Consumer Chemistry |

Electrochemistry |

Undergraduate Research |

Electrolytic / Galvanic Cells / Potentials |

Applications of Chemistry

Why Do I Have to Study Chemistry?G. Kenneth BarkerThis article is written from the point of view of a student in an introductory chemistry class for nonmajors. The student poses a long list of questions while going through his or her daily routine to prepare to go to class. Each question can be answered by the knowledge that would be gained in the class.Barker, G. Kenneth, Jr. J. Chem. Educ.2000, 77, 1300.

Consumer Chemistry |

Nonmajor Courses |

Applications of Chemistry

Understanding Electrochemical Thermodynamics through Entropy AnalysisThomas H. BindelThis discovery-based activity involves entropy analysis of galvanic cells. The intent of the activity is for students to discover the fundamentals of electrochemical cells through a combination of entropy analysis, exploration, and guided discovery. Bindel, Thomas H. J. Chem. Educ.2000, 77, 1031.

Electrochemistry |

Thermodynamics |

Electrolytic / Galvanic Cells / Potentials

Lemon Cells Revisited - The Lemon-Powered CalculatorDaniel J. Swartling and Charlotte MorganUsing lemons to create a voltaic cell to run items that students would use in their everyday lives drives home that chemistry plays an integral role in their lives. Swartling, Daniel J.; Morgan, Charlotte. J. Chem. Educ.1998, 75, 181.

Using the Biological Cell in Teaching ElectrochemistryMerkel, Eva Gankiewicz How electricity is produced in a simple cell is correlated with how commercial batteries work; this concept can then be related to how living cells send electrical impulses.Merkel, Eva Gankiewicz J. Chem. Educ.1994, 71, 240.

An industrial chemistry course: Bringing teachers and industry togetherFanning, James C.; Fanning, Sybil S.Local industry is able to supply direct examples of basic chemical principles that a teacher might use in classroom. The authors are eager to share their experiences, materials, lesson plans, etc., to prepare teachers to take their own classroom excursions to local industries.Fanning, James C.; Fanning, Sybil S. J. Chem. Educ.1993, 70, 563.

Using a projecting voltmeter to introduce voltaic cellsSolomon, Sally; Lee, Jeffrey; Schnable, Joseph; Wirtel, AnthonyUsing a transparent "projecting" voltmeter and assembling a zinc versus copper cell one component at a time allows students to develop a more concrete notion of the nature of a voltaic cell and the potential it produces.Solomon, Sally; Lee, Jeffrey; Schnable, Joseph; Wirtel, Anthony J. Chem. Educ.1989, 66, 510.

Experimental work with tin(II) chloride in a high school Sanchez, Manuela MartinThe author describes a final-project performed by students that integrates concepts of hydrolysis, Le Chatelier's principle, and electrolysis. Students seek answers to questions such as: "What reactions were involved; why is an aqueous solution of SnCl2 acidic; how can elemental tin be recovered from the system?" Sanchez, Manuela Martin J. Chem. Educ.1988, 65, 898.

Isolation of dyes for analysisLevinson, Alfred S.The use of ion exchange resin for the isolation of dyes from beverages, gelatin desserts, and other foods.Levinson, Alfred S. J. Chem. Educ.1977, 54, 460.

Car Won't Start?Nash, Leonard K.; Plumb, Robert C.Examines the questions, "Does the voltage of a battery drop with temperature" and "Does the ability of a battery to deliver current decrease with temperature?"Nash, Leonard K.; Plumb, Robert C. J. Chem. Educ.1970, 47, 382.

Electrochemistry |

Thin Layer Chromatography |

Applications of Chemistry |

Consumer Chemistry |

Electrolytic / Galvanic Cells / Potentials

The Becquerel effectEnsanian, MinasA short note on a demonstration of the Becquerel effect.Ensanian, Minas J. Chem. Educ.1968, 45, 240.